The answer is -33.6 degree Celsius... or approximately-34 degree Celsius. Firstly, you will change the L to mL so 2.10L to mL is 2100ML.. so if 750ML=-12 degree Celsius then 2100ML is what?? So.. if more less divide.. so 2100ML/750ML *-12 =-33.6 degree Celsius.. approximately -34 degree Celsius. I hope it helped??
<u>Answer: </u>
The pressure of a sample of argon gas was increased from 2.12atm to 6.96atm at constant temperature. If the final volume of the argon sample was 16.9L
. The initial volume of the argon sample was 55.5L
<u>Explanation:</u>
Considering the initial volume, initial pressure to be V1 and P1 respectively
Assuming the final volume and final temperature of the gas to be V2 and P2 respectively
Given,
Pressure of the gas was increased from 2.12 atm to 6.96 atm
Therefore, P1 = 2.12 atm
P2 = 6.96 atm
Final volume, V2 = 16.9 L
Applying Boyle’s law,
Substituting the value
V1 = 55.5 L
Therefore, the initial volume was 55.5L
C. Increasing the volume of gas particles of H2 and I2 will decrease the rate of the forward reaction. As the gas particles will not undergo frequent collisions as much and thus will not produce as much product.